Question

Arrange the following compounds in increasing order of their ionic character.
\[SnC{l_2},\,SnC{l_4},\,SiC{l_4},\,Sn{F_4},\,Sn{F_2}\]
A. \[Sn{F_2} < SnC{l_2} < SnC{l_4} < SiC{l_4}\]
B. \[Sn{F_2} < SnC{l_2} < SiC{l_4} < SnC{l_4}\]
C. \[Sn{F_2} < SnC{l_2} < SnC{l_4} < Si{F_2}\]
D. \[Sn{F_2} < SnC{l_2} < Sn{F_4} < SiC{l_4}\]

Answer 1

Hint: Ionic compounds have greater melting and boiling points because their molecules attract one another more strongly. As a lattice energy is defined as the force needed to separate an ionic compound into its individual gaseous ions. The stronger the bond, the more lattice energy will be present.

Complete Step-by-Step Explanation:
In order to know the lattice energies of the ionic compounds that are relatively high. For instance, the lattice energy of \[NaCl\] is \[787.3\,KJ/mol\], which is just a tiny amount of the energy released during gas combustion. When the ions are tiny, the binding between ions with opposite charges is strongest. Compare the given compound series to \[SnC{l_4}\]and \[SnC{l_2}\]which have high melting points. Also keep in mind that a metal cation's polarising effect grows as its charge does, that is giving the molecule a covalent property.
\[SnC{l_4}\] will be covalent and \[SnC{l_2}\] will be ionic. Therefore, the charges on the ions and, consequently, the separation between the centres of the ions after they pack to form a crystal, determine the strength of the connection between the ions of opposite charge in an ionic compound. The lattice energy of the compound, or the energy released when oppositely charged ions inside the gas phase close to form a solid, can be used to determine the strength of the bonds in an ionic compound.
So, the lattice energy of the ionic character is: \[Sn{F_2} < SnC{l_2} < SnC{l_4} < SiC{l_4}\]and the lattice enthalpy is: \[Sn{F_2} > SnC{l_2} > SnC{l_4} > SiC{l_4}\]because lattice enthalpy is directly proportional to the covalent characters of the compound.

Thus, the correct option is: (A) \[Sn{F_2} < SnC{l_2} < SnC{l_4} < SiC{l_4}\]

Note: It should be noted that a crystal structure also affects lattice energy Because the ionic radii of the cations decrease in the order and there are some additional considerations to be aware of, such as covalent character and electron-electron interactions from lithium to potassium, the lattice energy gradually decreases. In contrast, the iodide salt always has a very low lattice energy and the fluoride compound always has the highest for a given metallic element ion.